DAT General Chemistry Equation Sheet

Chapter 0: General and Lab Concepts Review

Dilutions

𝑀1𝑉1=𝑀2𝑉2 or

𝐶1𝑉1=𝐶2𝑉2

𝑀 𝑜𝑟 𝐶= 𝑐 𝑜𝑛𝑐𝑒𝑛𝑡𝑟𝑎𝑡𝑖𝑜𝑛

𝑉=𝑣𝑜𝑙𝑢𝑚𝑒

Percent Error

(𝐴−𝑇)

𝑇×100

𝑇=𝑡ℎ𝑒𝑜𝑟𝑒𝑡𝑖𝑐𝑎𝑙

𝐴=𝑎𝑐𝑡𝑢𝑎𝑙

Absorbance

(Spectro-

photometer)

𝐴𝑏𝑠=𝜀𝑐𝑙

𝜀 =𝑚𝑜𝑙𝑎𝑟 𝑒𝑥𝑡𝑖𝑛𝑐𝑡𝑖𝑜𝑛

𝑐𝑜𝑒𝑓𝑓𝑖𝑐𝑖𝑒𝑛𝑡 (𝑚𝑜𝑙𝑎𝑟

𝑎𝑏𝑠𝑜𝑟𝑝𝑡𝑖𝑣𝑖𝑡𝑦)

𝑐=𝑠𝑎𝑚𝑝𝑙𝑒′𝑠 𝑐𝑜𝑛𝑐𝑒𝑛𝑡𝑟𝑎𝑡𝑖𝑜𝑛

𝑙=𝑝𝑎𝑡ℎ 𝑙𝑒𝑛𝑔𝑡ℎ

Chapter 2: Atomic and Electronic Structure

Energy of a

photon

𝐸𝑝ℎ𝑜𝑡𝑜𝑛 =ℎ𝑓=ℎ𝑐

𝜆

ℎ=𝑃𝑙𝑎𝑛𝑐𝑘′𝑠 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡

(6.63×10−34𝐽∙𝑠)

𝑓=𝑝ℎ𝑜𝑡𝑜𝑛′𝑠 𝑓𝑟𝑒𝑞𝑢𝑒𝑛𝑐𝑦

𝑐 =𝑠𝑝𝑒𝑒𝑑 𝑜𝑓 𝑙𝑖𝑔ℎ𝑡

(3.0×108𝑚𝑠

⁄)

𝜆=𝑝ℎ𝑜𝑡𝑜𝑛′𝑠

𝑤𝑎𝑣𝑒𝑙𝑒𝑛𝑔𝑡ℎ

Absorption/

Emission Line

Spectra

𝛥𝐸=𝐸𝑝ℎ𝑜𝑡𝑜𝑛

Kinetic Energy

of an electron

(Photoelectric

Effect)

𝐾𝐸𝑒− =𝐸𝑝ℎ𝑜𝑡𝑜𝑛 −𝜙

𝜙 =𝑤𝑜𝑟𝑘 𝑓𝑢𝑛𝑐𝑡𝑖𝑜𝑛

(𝑚𝑖𝑛𝑖𝑚𝑢𝑚 𝑒𝑛𝑒𝑟𝑔𝑦 𝑛𝑒𝑒𝑑𝑒𝑑

𝑡𝑜 𝑖𝑜𝑛𝑖𝑧𝑒 𝑒𝑙𝑒𝑐𝑡𝑟𝑜𝑛)

Chapter 7: Chemical Solutions

Molarity

𝑀=𝑚𝑜𝑙𝑒𝑠𝑠𝑜𝑙𝑢𝑡𝑒

𝐿𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛

Molality

𝑚=𝑚𝑜𝑙𝑒𝑠𝑠𝑜𝑙𝑢𝑡𝑒

𝑘𝑔𝑠𝑜𝑙𝑣𝑒𝑛𝑡

Henry’s

Law

𝑃𝐴=𝑘𝐻[𝐴]

𝑃𝐴=𝑝𝑎𝑟𝑡𝑖𝑎𝑙 𝑝𝑟𝑒𝑠𝑠𝑢𝑟𝑒 𝑜𝑓 𝑔𝑎𝑠 𝐴

𝑘𝐻=𝐻𝑒𝑛𝑟𝑦′𝑠 𝐿𝑎𝑤 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡

(𝑣𝑎𝑟𝑖𝑒𝑠 𝑝𝑒𝑟 𝑝𝑟𝑜𝑏𝑙𝑒𝑚)

[A] = conc. of gas A

Freezing

Point

Depression

𝛥𝑇𝐹=−𝑖𝐾𝐹𝑚

𝑖=𝑣𝑎𝑛′𝑡 𝐻𝑜𝑓𝑓 𝑓𝑎𝑐𝑡𝑜𝑟

𝐾𝐹= 𝐹. 𝑃. 𝑑𝑒𝑝𝑟𝑒𝑠𝑠𝑖𝑜𝑛 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡

𝑚=𝑚𝑜𝑙𝑎𝑙𝑖𝑡𝑦

Boiling

Point

Elevation

𝛥𝑇𝐵=𝑖𝐾𝐵𝑚

𝑖=𝑣𝑎𝑛′𝑡 𝐻𝑜𝑓𝑓 𝑓𝑎𝑐𝑡𝑜𝑟

𝐾𝐵= 𝐵. 𝑃.𝑑 𝑒𝑝𝑟𝑒𝑠𝑠𝑖𝑜𝑛 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡

𝑚=𝑚𝑜𝑙𝑎𝑙𝑖𝑡𝑦

Vapor

Pressure

Depression

(Raoult’s

Law)

𝑃𝑠𝑜𝑙𝑛 =𝜒𝑠𝑜𝑙𝑣𝑃𝑠𝑜𝑙𝑣0

𝑃𝑠𝑜𝑙𝑛 = 𝑉𝑃 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛

𝜒𝑠𝑜𝑙𝑣 = 𝑚𝑜𝑙 𝑓𝑟𝑎𝑐𝑡 𝑜𝑓 𝑠𝑜𝑙𝑣𝑒𝑛𝑡

𝑃𝑠𝑜𝑙𝑣0= 𝑉𝑃 𝑜𝑓 𝑝𝑢𝑟𝑒 𝑠𝑜𝑙𝑣𝑒𝑛𝑡

Osmotic

Pressure

(𝝅)

𝜋=𝑖𝑀𝑅𝑇

𝑀 =𝑚𝑜𝑙𝑎𝑟𝑖𝑡𝑦 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒

𝑖=𝑣𝑎𝑛′𝑡 𝐻𝑜𝑓𝑓 𝑓𝑎𝑐𝑡𝑜𝑟

𝑅 = 0 .0821 𝐿⋅𝑎𝑡𝑚

𝑚𝑜𝑙⋅𝐾

𝑇=𝑡𝑒𝑚𝑝.𝑖𝑛 𝐾𝑒𝑙𝑣𝑖𝑛

Chapter 5: Gases

Pressure

𝑃=𝐹

𝐴

𝐹=𝑓𝑜𝑟𝑐𝑒

𝐴=𝑎𝑟𝑒𝑎

Average Kinetic

Energy

𝐾𝐸𝑎𝑣𝑔 = 32

⁄𝑅𝑇

𝑅=8.314 𝐽

𝑚𝑜𝑙∙𝐾

Root-Mean-

Square Speed

(𝒗)

𝑣 = √3𝑅𝑇

𝑀𝑚

𝑅=8.314 𝐽

𝑚𝑜𝑙∙𝐾

𝑀𝑚= 𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠

Ideal Gas Law

𝑃𝑉=𝑛𝑅𝑇

𝑛 =# 𝑜𝑓 𝑚𝑜𝑙𝑒𝑠

𝑅 =0.0821 𝐿⋅𝑎𝑡𝑚

𝑚𝑜𝑙⋅𝐾

Boyle’s Law

𝑉∝1

𝑃

Charles’ Law

𝑉∝𝑇

Avogadro’s Law

𝑉∝𝑛

Combined Gas

Law

𝑃1𝑉1

𝑛1𝑇1=𝑃2𝑉2

𝑛2𝑇2

Standard Temp.

& Pressure (STP)

P=1 atm

T=273 K

*1 mol of gas = 22.4 L

at STP

Standard

Conditions

All aqueous species @ 1M

All gaseous species @1 atm

T=298 K

Density

𝑃(𝑀𝑀)

𝑅𝑇 =𝑚

𝑣

𝑀𝑀=𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠

𝑅 =0.0821 𝐿⋅𝑎𝑡𝑚

𝑚𝑜𝑙⋅𝐾

𝑚=𝑚𝑎𝑠𝑠

𝑣=𝑣𝑜𝑙𝑢𝑚𝑒

Dalton’s Law of

Partial Pressures

𝑃𝑡𝑜𝑡𝑎𝑙 =𝑃𝐴+𝑃𝐵+⋯

Dalton’s Law of

Partial Pressures

𝑃𝐴=𝜒𝐴𝑃𝑡𝑜𝑡𝑎𝑙

𝜒𝐴= 𝑚𝑜𝑙 𝑓𝑟𝑎𝑐𝑡𝑖𝑜𝑛

𝑜𝑓 𝑔𝑎𝑠 𝐴

Graham’s Law of

Effusion

𝑟1

𝑟2=√𝑀𝑚2

𝑀𝑚1

𝑟 =𝑟𝑎𝑡𝑒 𝑜𝑓 𝑒𝑓𝑓𝑢𝑠𝑖𝑜𝑛

𝑀 =𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠

Real Gas

Equation

(𝑃+𝑎𝑛2

𝑉2)(𝑉

−𝑛𝑏)=𝑛𝑅𝑇

𝑎 & 𝑏 =𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡𝑠

𝑠𝑝𝑒𝑐𝑖𝑓𝑖𝑐 𝑡𝑜 𝑒𝑎𝑐ℎ 𝑔𝑎𝑠

𝑎𝑛2

𝑉2 𝑐𝑜𝑟𝑟𝑒𝑐𝑡𝑠 𝑓𝑜𝑟

𝐼𝑀𝐹𝑠

−𝑛𝑏 𝑐𝑜𝑟𝑟𝑒𝑐𝑡𝑠 𝑓𝑜𝑟

𝑣𝑜𝑙𝑢𝑚𝑒

Chapter 8: Chemical Kinetics

General

Rate Law

A + B → C + D

𝑟𝑎𝑡𝑒=𝑘[𝐴]𝑚[𝐵]𝑛

𝑘 =𝑟𝑎𝑡𝑒 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡

𝑚 & 𝑛 =𝑑𝑒𝑡𝑒𝑟𝑚𝑖𝑛𝑒𝑑

e𝑥𝑝𝑒𝑟𝑖𝑚𝑒𝑛𝑡𝑎𝑙𝑙𝑦

Rate

Constant

Units

0 𝑜𝑟𝑑𝑒𝑟: 𝑘 = 𝑀1∙𝑠−1

1𝑠𝑡 𝑜𝑟𝑑𝑒𝑟: 𝑘 =𝑠 −1

2𝑛𝑑 𝑜𝑟𝑑𝑒𝑟: 𝑘=𝑀−1∙𝑠−1

3𝑟𝑑 𝑜𝑟𝑑𝑒𝑟: 𝑘=𝑀−2∙𝑠−1

𝑘 =𝑟𝑎𝑡𝑒 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡

𝑀=𝑚𝑜𝑙𝑎𝑟𝑖𝑡𝑦

s=𝑠𝑒𝑐𝑜𝑛𝑑𝑠

Arrhenius

Equation

𝑘=𝐴𝑒−𝐸𝑎𝑅𝑇

⁄

𝑘 =𝑟𝑎𝑡𝑒 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡

𝐴 = 𝑢𝑛𝑖𝑞𝑢𝑒 𝑡𝑜 𝑒𝑎𝑐ℎ 𝑟𝑥𝑛

𝐸𝑎=𝑎𝑐𝑡.𝑒𝑛𝑒𝑟𝑔𝑦

𝑅=8.314 𝐽

𝑚𝑜𝑙∙𝐾

𝑇=𝑡𝑒𝑚𝑝.𝑖𝑛 𝐾𝑒𝑙𝑣𝑖𝑛

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DAT General Chemistry Equation Sheet

Chapter 0: General and Lab Concepts Review

Dilutions 𝑀 1 𝑉 1 = 𝑀 2 𝑉 2 or

Percent Error (𝐴^ −^ 𝑇)

× 100

Absorbance

(Spectro-

photometer)

𝐴𝑏𝑠 = 𝜀𝑐𝑙 𝜀^ =^ 𝑚𝑜𝑙𝑎𝑟^ 𝑒𝑥𝑡𝑖𝑛𝑐𝑡𝑖𝑜𝑛

Chapter 2: Atomic and Electronic Structure

Energy of a

photon

( 6. 63 × 10 −^34 𝐽 ∙ 𝑠)

( 3. 0 × 108 𝑚⁄^ 𝑠^ )

Absorption/

Emission Line

Spectra

Kinetic Energy

of an electron

(Photoelectric

Effect)

𝐾𝐸𝑒− = 𝐸𝑝ℎ𝑜𝑡𝑜𝑛 − 𝜙 𝜙^ =^ 𝑤𝑜𝑟𝑘^ 𝑓𝑢𝑛𝑐𝑡𝑖𝑜𝑛

Chapter 7: Chemical Solutions

Molarity

Molality

Henry’s

Law

𝑃𝐴 = 𝑘𝐻 [𝐴] 𝑃𝐴^ =^ 𝑝𝑎𝑟𝑡𝑖𝑎𝑙^ 𝑝𝑟𝑒𝑠𝑠𝑢𝑟𝑒^ 𝑜𝑓^ 𝑔𝑎𝑠^ 𝐴

[A] = conc. of gas A

Freezing

Point

Depression

𝛥𝑇𝐹 = −𝑖𝐾𝐹 𝑚 𝑖^ =^ 𝑣𝑎𝑛′𝑡^ 𝐻𝑜𝑓𝑓^ 𝑓𝑎𝑐𝑡𝑜𝑟

Boiling

Point

Elevation

𝛥𝑇𝐵 = 𝑖𝐾𝐵 𝑚 𝑖^ =^ 𝑣𝑎𝑛′𝑡^ 𝐻𝑜𝑓𝑓^ 𝑓𝑎𝑐𝑡𝑜𝑟

Vapor

Pressure

Depression

(Raoult’s

Law)

𝑃𝑠𝑜𝑙𝑛 = 𝜒𝑠𝑜𝑙𝑣 𝑃𝑠𝑜𝑙𝑣 0 𝑃𝑠𝑜𝑙𝑛^ =^ 𝑉𝑃^ 𝑜𝑓^ 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛

𝑃𝑠𝑜𝑙𝑣^0 = 𝑉𝑃 𝑜𝑓 𝑝𝑢𝑟𝑒 𝑠𝑜𝑙𝑣𝑒𝑛𝑡

Osmotic

Pressure

𝜋 = 𝑖𝑀𝑅𝑇 𝑀^ =^ 𝑚𝑜𝑙𝑎𝑟𝑖𝑡𝑦^ 𝑜𝑓^ 𝑠𝑜𝑙𝑢𝑡𝑒

𝑅 = 0. 0821 𝐿 ⋅ 𝑎𝑡𝑚 𝑚𝑜𝑙 ⋅ 𝐾 𝑇 = 𝑡𝑒𝑚𝑝. 𝑖𝑛 𝐾𝑒𝑙𝑣𝑖𝑛

Chapter 5: Gases

Pressure

Average Kinetic

Energy

𝐾𝐸𝑎𝑣𝑔 = 3 ⁄^2 𝑅𝑇 𝑅 = 8. 314 𝐽

Root-Mean-

Square Speed

Ideal Gas Law 𝑃𝑉 = 𝑛𝑅𝑇 𝑛^ =^ #^ 𝑜𝑓^ 𝑚𝑜𝑙𝑒𝑠

Boyle’s Law

Charles’ Law 𝑉 ∝ 𝑇

Avogadro’s Law 𝑉 ∝ 𝑛

Combined Gas

Law

Standard Temp.

& Pressure (STP)

P=1 atm

T=273 K

*1 mol of gas = 22.4 L at STP

Standard

Conditions

All aqueous species @ 1M

All gaseous species @1 atm

T=298 K

Density 𝑃(𝑀𝑀)

Dalton’s Law of

Partial Pressures

Dalton’s Law of

Partial Pressures

𝑃𝐴 = 𝜒𝐴𝑃𝑡𝑜𝑡𝑎𝑙 𝜒𝐴 =^ 𝑚𝑜𝑙^ 𝑓𝑟𝑎𝑐𝑡𝑖𝑜𝑛

Graham’s Law of

Effusion

Real Gas

Equation (𝑃^ +^

𝑎𝑛^2

𝑉^2

𝑎𝑛^2

𝑉^2

Chapter 8: Chemical Kinetics

General

Rate Law

A + B → C + D

𝑟𝑎𝑡𝑒 = 𝑘[𝐴]𝑚[𝐵]𝑛

e𝑥𝑝𝑒𝑟𝑖𝑚𝑒𝑛𝑡𝑎𝑙𝑙𝑦

Rate

Constant

Units

0 𝑜𝑟𝑑𝑒𝑟: 𝑘 = 𝑀^1 ∙ 𝑠−^1

1 𝑠𝑡^ 𝑜𝑟𝑑𝑒𝑟: 𝑘 = 𝑠−^1

2 𝑛𝑑^ 𝑜𝑟𝑑𝑒𝑟: 𝑘 = 𝑀−^1 ∙ 𝑠−^1

3 𝑟𝑑^ 𝑜𝑟𝑑𝑒𝑟: 𝑘 = 𝑀−^2 ∙ 𝑠−^1

s= 𝑠𝑒𝑐𝑜𝑛𝑑𝑠

Arrhenius

Equation

𝑘 = 𝐴𝑒−𝐸𝑎^ ⁄𝑅𝑇^ 𝑘^ =^ 𝑟𝑎𝑡𝑒^ 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡

DAT General Chemistry Equation Sheet Chapter 12: Electrochemistry & Redox Reactions

Standard

Cell

Potential

Nernst

Equation

log 𝑄

t𝑟𝑎𝑛𝑠𝑓𝑒𝑟𝑟𝑒𝑑 𝑄 = 𝑟𝑒𝑎𝑐𝑡𝑖𝑜𝑛 𝑞𝑢𝑜𝑡𝑖𝑒𝑛𝑡

Faraday’s

Law

𝐼 = 𝑐𝑢𝑟𝑟𝑒𝑛𝑡 (Amps) 𝑡𝑠 = 𝑡𝑖𝑚𝑒 (𝑠𝑒𝑐𝑜𝑛𝑑𝑠) 𝑛 = # 𝑜𝑓 𝑒𝑙𝑒𝑐𝑡𝑟𝑜𝑛𝑠 𝑡𝑟𝑎𝑛𝑠𝑓𝑒𝑟𝑟𝑒𝑑 𝐹 = 𝐹𝑎𝑟𝑎𝑑𝑎𝑦′𝑠 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡 ( 96485

𝑚𝑜𝑙 𝑒−^ )

Chapter 9: Chemical Equilibria

Equilibrium

Constant

Expressions

𝐾𝑐 = [[𝑟𝑒𝑎𝑐𝑡𝑎𝑛𝑡𝑠𝑝𝑟𝑜𝑑𝑢𝑐𝑡𝑠]]

𝑃𝑝𝑟𝑜𝑑𝑢𝑐𝑡𝑠 𝑃𝑟𝑒𝑎𝑐𝑡𝑎𝑛𝑡𝑠

Reaction

Quotient (Q)

[𝑝𝑟𝑜𝑑𝑢𝑐𝑡𝑠]

[𝑟𝑒𝑎𝑐𝑡𝑎𝑛𝑡𝑠]

Solubility

Product

Constant ( 𝑲𝒔𝒑)

[𝑝𝑟𝑜𝑑𝑢𝑐𝑡𝑠]

[𝑟𝑒𝑎𝑐𝑡𝑎𝑛𝑡𝑠]

Chapter 10: Acid-Base Equilbria & Titrations

Ionization

Constant

of Water

𝐾𝑤 = [𝐻 3 𝑂+][ 𝑂𝐻−] = 1 × 10 −^14

@ 25 °C

pH & pOH 𝑝𝐻 = −log[𝐻+]

𝑝𝑂𝐻 = −log[𝑂𝐻−]

[𝐻+]

[𝑂𝐻−]

[H+] &

[OH-]

[𝐻+] = 10 −𝑝𝐻

[𝑂𝐻−] = 10 −𝑝𝐻

[𝐻+][𝑂𝐻−] = 1 ∗ 10 −^14

Weak

Acids

𝐻𝐴 + 𝐻 2 𝑂 ⇌ 𝐻 3 𝑂+^ + 𝐴−

[𝐻 3 𝑂+][𝐴−]

[𝐻𝐴]

[𝐻+] = √𝐾𝑎[𝐻𝐴]

Weak

Bases

𝐴−^ + 𝐻 2 𝑂 ⇌ 𝐻𝐴 + 𝑂𝐻−

[𝑂𝐻−][𝐻𝐴]

[𝐴−]

[𝑂𝐻−] = √𝐾𝑏 [𝐴−]

pKa & pKb 𝑝𝐾𝑎 = −log[𝐾𝑎]

𝑝𝐾𝑏 = −log[𝐾𝑏]

𝐾𝑤 = 𝐾𝑎 × 𝐾𝑏 = 1

∗ 10 −^14

Larger 𝐾𝑎 = smaller p𝐾𝑎 =stronger acid Larger 𝐾𝑏 = smaller p𝐾𝑏 =stronger base Neutralization

Reaction

𝑛𝐴𝑀𝐴𝑉𝐴 = 𝑛𝐵 𝑀𝐵 𝑉𝐵 𝑛𝐴 =^ #^ 𝑜𝑓^ 𝑚𝑜𝑙𝑒𝑠^ 𝐻+

Buffers

𝑝𝐻 = 𝑝𝐾𝑎 + log

[𝐴−]

[𝐻𝐴]

[𝐴−] = 𝑐𝑜𝑛𝑐. 𝑜𝑓 𝑏𝑎𝑠𝑒

[𝐻𝐴] = 𝑐𝑜𝑛𝑐. 𝑜𝑓 𝑎𝑐𝑖𝑑

Chapter 13: Nuclear Reactions

Kinetics

(always 1st

order)

𝑁 = 𝑁 0 𝑒−𝑘𝑡 ln 𝑁 = ln 𝑁 0 − 𝑘𝑡 𝑡 1 / 2 =

693 𝑘

*note that 𝑡 1 / 2 is independent of concn for 1st^ order rxns

Nuclear

Binding

Energy

𝐸 = 𝛥𝑚𝑐^2 𝑚^ =^ 𝑚𝑎𝑠𝑠^ (𝑀𝑈𝑆𝑇^ 𝑏𝑒^ 𝑖𝑛^ 𝑘𝑔) 𝑐 = 𝑠𝑝𝑒𝑒𝑑 𝑜𝑓 𝑙𝑖𝑔ℎ𝑡 ( 3. 0 × 108

Chapter 11: Thermodynamics & Thermochemistry

Enthalpy (H) (𝛥𝐻 > 0 ): 𝑒𝑛𝑑𝑜𝑡ℎ𝑒𝑟𝑚𝑖𝑐

Enthalpy of

Formation

First Law of

Thermo-

dynamics

𝛥𝐸 = 𝑞 + 𝑤 𝛥𝐸^ =^ 𝑐ℎ𝑎𝑛𝑔𝑒^ 𝑖𝑛^ 𝑖𝑛𝑡𝑒𝑟𝑛𝑎𝑙 𝑒𝑛𝑒𝑟𝑔𝑦 𝑞 = ℎ𝑒𝑎𝑡 𝑤 = 𝑤𝑜𝑟𝑘

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DAT General Chemistry Equation Sheet

Chapter 0: General and Lab Concepts Review

Dilutions 𝑀 1 𝑉 1 = 𝑀 2 𝑉 2 or

Percent Error (𝐴^ −^ 𝑇)

× 100

Absorbance

(Spectro-

photometer)

𝐴𝑏𝑠 = 𝜀𝑐𝑙 𝜀^ =^ 𝑚𝑜𝑙𝑎𝑟^ 𝑒𝑥𝑡𝑖𝑛𝑐𝑡𝑖𝑜𝑛

Chapter 2: Atomic and Electronic Structure

Energy of a

photon

( 6. 63 × 10 −^34 𝐽 ∙ 𝑠)

( 3. 0 × 108 𝑚⁄^ 𝑠^ )

Absorption/

Emission Line

Spectra

Kinetic Energy

of an electron

(Photoelectric

Effect)

𝐾𝐸𝑒− = 𝐸𝑝ℎ𝑜𝑡𝑜𝑛 − 𝜙 𝜙^ =^ 𝑤𝑜𝑟𝑘^ 𝑓𝑢𝑛𝑐𝑡𝑖𝑜𝑛

Chapter 7: Chemical Solutions

Molarity

Molality

Henry’s

Law

𝑃𝐴 = 𝑘𝐻 [𝐴] 𝑃𝐴^ =^ 𝑝𝑎𝑟𝑡𝑖𝑎𝑙^ 𝑝𝑟𝑒𝑠𝑠𝑢𝑟𝑒^ 𝑜𝑓^ 𝑔𝑎𝑠^ 𝐴

Freezing

Point

Depression

𝛥𝑇𝐹 = −𝑖𝐾𝐹 𝑚 𝑖^ =^ 𝑣𝑎𝑛′𝑡^ 𝐻𝑜𝑓𝑓^ 𝑓𝑎𝑐𝑡𝑜𝑟

Boiling

Point

Elevation

𝛥𝑇𝐵 = 𝑖𝐾𝐵 𝑚 𝑖^ =^ 𝑣𝑎𝑛′𝑡^ 𝐻𝑜𝑓𝑓^ 𝑓𝑎𝑐𝑡𝑜𝑟

Vapor

Pressure

Depression

(Raoult’s

Law)

𝑃𝑠𝑜𝑙𝑛 = 𝜒𝑠𝑜𝑙𝑣 𝑃𝑠𝑜𝑙𝑣 0 𝑃𝑠𝑜𝑙𝑛^ =^ 𝑉𝑃^ 𝑜𝑓^ 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛

𝑃𝑠𝑜𝑙𝑣^0 = 𝑉𝑃 𝑜𝑓 𝑝𝑢𝑟𝑒 𝑠𝑜𝑙𝑣𝑒𝑛𝑡

Osmotic

Pressure

𝜋 = 𝑖𝑀𝑅𝑇 𝑀^ =^ 𝑚𝑜𝑙𝑎𝑟𝑖𝑡𝑦^ 𝑜𝑓^ 𝑠𝑜𝑙𝑢𝑡𝑒

Chapter 5: Gases

Pressure

Average Kinetic

Energy

𝐾𝐸𝑎𝑣𝑔 = 3 ⁄^2 𝑅𝑇 𝑅 = 8. 314 𝐽

Root-Mean-

Square Speed

Ideal Gas Law 𝑃𝑉 = 𝑛𝑅𝑇 𝑛^ =^ #^ 𝑜𝑓^ 𝑚𝑜𝑙𝑒𝑠

Boyle’s Law

Charles’ Law 𝑉 ∝ 𝑇

Avogadro’s Law 𝑉 ∝ 𝑛

Combined Gas

Law

Standard Temp.

& Pressure (STP)

P=1 atm

T=273 K

Standard

Conditions

All aqueous species @ 1M

All gaseous species @1 atm

T=298 K

Density 𝑃(𝑀𝑀)

Dalton’s Law of

Partial Pressures

Dalton’s Law of

Partial Pressures

𝑃𝐴 = 𝜒𝐴𝑃𝑡𝑜𝑡𝑎𝑙 𝜒𝐴 =^ 𝑚𝑜𝑙^ 𝑓𝑟𝑎𝑐𝑡𝑖𝑜𝑛

Graham’s Law of